Objectives After studying this Unit, you will be able to • explain the terms minerals, ores, concentration, benefaction, calcination, roasting, refining, etc.; • understand the principles of oxidation and reduction as applied to the extraction procedures; • apply the thermodynamic concepts like that of Gibbs energy and entropy to the principles of extraction of Al, Cu, Zn and Fe; • explain why reduction of certain oxides like Cu2O is much easier than that of Fe2O3; • explain why CO is a favourable reducing agent at certain temperatures while coke is better in some other cases; • explain why specific reducing agents are used for the reduction purposes. Thermodynamics illustrates why only a certain reducing element and a minimum specific temperature are suitable for reduction of a metal oxide to the metal in an extraction. A few elements like carbon, sulphur, gold and noble gases, occur in free state while others in combined forms in the earth’s crust. The extraction and isolation of an element from its combined form involves various principles of chemistry. A particular element may occur in a variety of compounds. The process of metallurgy and isolation should be such that it is chemically feasible and commercially viable. Still, some general principles are common to all the extraction processes of metals. For obtaining a particular metal, first we look for minerals which are naturally occurring chemical substances in the earth’s crust obtainable by mining. Out of many minerals in which a metal may be found, only a few are viable to be used as sources of that metal. Such minerals are known as ores. Rarely, an ore contains only a desired substance. It is usually contaminated with earthly or undesired materials known as gangue. The extraction and isolation of metals from ores involve the following major steps: • Concentration of the ore, • Isolation of the metal from its concentrated ore, and • Purification of the metal. The entire scientific and technological process used for isolation of the metal from its ores is known as metallurgy. 6.1 Occurrence of Metals In the present Unit, first we shall describe various steps for effective concentration of ores. After that we shall discuss the principles of some of the common metallurgical processes. Those principles shall include the thermodynamic and electrochemical aspects involved in the effective reduction of the concentrated ore to the metal. Elements vary in abundance. Among metals, aluminium is the most abundant. It is the third most abundant element in earth’s crust (8.3% approx. by weight). It is a major component of many igneous minerals including mica and clays. Many gemstones are impure forms of Al2O3 and the impurities range from Cr (in ‘ruby’) to Co (in ‘sapphire’). Iron is the second most abundant metal in the earth’s crust. It forms a variety of compounds and their various uses make it a very important element. It is one of the essential elements in biological systems as well. The principal ores of aluminium, iron, copper and zinc have been given in Table 6.1. 6.2 Concentration of Ores 6.2.1 Hydraulic Washing For the purpose of extraction, bauxite is chosen for aluminium. For iron, usually the oxide ores which are abundant and do not produce polluting gases (like SO2 that is produced in case iron pyrites) are taken. For copper and zinc, any of the listed ores (Table 6.1) may be used depending upon availability and other relevant factors. Before proceeding for concentration, ores are graded and crushed to reasonable size. Removal of the unwanted materials (e.g., sand, clays, etc.) from the ore is known as concentration, dressing or benefaction. It involves several steps and selection of these steps depends upon the differences in physical properties of the compound of the metal present and that of the gangue. The type of the metal, the available facilities and the environmental factors are also taken into consideration. Some of the important procedures are described below. This is based on the differences in gravities of the ore and the gangue particles. It is therefore a type of gravity separation. In one such process, an upward stream of running water is used to wash the powdered ore. The lighter gangue particles are washed away and the heavier ores are left behind. 6.2.2 Magnetic This is based on differences in Separation magnetic properties of the ore components. If either the ore or the gangue (one of these two) is capable of being attracted by a magnetic field, then such separations are carried out (e.g., in case of iron ores). The ground ore is carried on a conveyer belt which passes over a Fig. 6.1: Magnetic separation (schematic)magnetic roller (Fig.6.1). 6.2.3 Froth This method has been in use for removing gangue from sulphide ores. In Floatation this process, a suspension of the powdered ore is made with water. To it, Method collectors and froth stabilisers are added. Collectors (e. g., pine oils, fatty acids, xanthates, etc.) enhance non-wettability of the mineral particles and froth stabilisers (e. g., cresols, aniline) stabilise the froth. The mineral particles become wet by oils while the gangue particles by water. A rotating paddle agitates the mixture and draws air in it. As a result, froth is formed which carries the mineral particles. The froth is light and is skimmed off. It is then dried for recovery of the ore particles. Sometimes, it is possible to separate two sulphide ores by adjusting proportion of oil to water or by using ‘depressants’. For example, in case of an ore containing ZnS and PbS, the depressant used is NaCN. It selectively prevents ZnS from coming to the Fig. 6.2: Froth floatation process (schematic) froth but allows PbS to come with the froth. The Innovative Washerwoman One can do wonders if he or she has a scientific temperament and is attentive to observations. A washerwoman had an innovative mind too. While washing a miner’s overalls, she noticed that sand and similar dirt fell to the bottom of the washtub. What was peculiar, the copper bearing compounds that had come to the clothes from the mines, were caught in the soapsuds and so they came to the top. One of her clients was a chemist, Mrs. Carrie Everson. The washerwoman told her experience to Mrs. Everson. The latter thought that the idea could be used for separating copper compounds from rocky and earth materials on large scale. This way an invention was born. At that time only those ores were used for extraction of copper, which contained large amounts of the metal. Invention of the Froth Floatation Method made copper mining profitable even from the low-grade ores. World production of copper soared and the metal became cheaper. 6.2.4 Leaching Leaching is often used if the ore is soluble in some suitable solvent. The following examples illustrate the procedure: (a) Leaching of alumina from bauxite The principal ore of aluminium, bauxite, usually contains SiO2, iron oxides and titanium oxide (TiO2) as impurities. Concentration is carried out by digesting the powdered ore with a concentrated solution of NaOH at 473 – 523 K and 35 – 36 bar pressure. This way, Al2O3 is leached out as sodium aluminate (and SiO2 too as sodium silicate) leaving the impurities behind: Al2O3(s) + 2NaOH(aq) + 3H2O(l) → 2Na[Al(OH) 4](aq) (6.1) The aluminate in solution is neutralised by passing CO2 gas and hydrated Al2O3 is precipitated. At this stage, the solution is seeded with freshly prepared samples of hydrated Al2O3 which induces the precipitation: 2Na[Al(OH)4](aq) + CO2(g) → Al2O3.xH2O(s) + 2NaHCO3 (aq) (6.2) The sodium silicate remains in the solution and hydrated alumina is filtered, dried and heated to give back pure Al2O3: 1470 KAl2O3.xH2O(s) Al2O3(s) + xH2O(g) (6.3) (b) Other examples In the metallurgy of silver and that of gold, the respective metal is leached with a dilute solution of NaCN or KCN in the presence of air (for O2) from which the metal is obtained later by replacement: 4M(s) + 8CN–(aq)+ 2H2O(aq) + O2(g) → 4[M(CN)2]– (aq) +4OH –(aq) (M= Ag or Au) (6.4) − 2−2M() aq +Zn()→Zn() aq +2M() (6.5)[ CN 2 ]( ) s [ CN 4 ]( ) s 6.3 Extraction of Crude Metal from Concentrated Ore The concentrated ore must be converted into a form which is suitable for reduction. Usually the sulphide ore is converted to oxide before reduction. Oxides are easier to reduce (for the reason see box). Thus isolation of metals from concentrated ore involves two major steps viz., (a) conversion to oxide, and (b) reduction of the oxide to metal. (a) Conversion to oxide (i) Calcination: Calcinaton involves heating when the volatile matter escapes leaving behind the metal oxide: Fe2O3.xH2O(s) �Fe2O3 (s) + xH2O(g) (6.6) ZnCO3 (s) �ZnO(s) + CO2(g) (6.7) CaCO3.MgCO3(s) �CaO(s) + MgO(s ) + 2CO2(g) (6.8) 6.4 Thermodynamic Principles of Metallurgy (ii) Roasting: In roasting, the ore is heated in a regular supply of air in a furnace at a temperature below the melting point of the metal. Some of the reactions involving sulphide ores are: 2ZnS + 3O2 → 2ZnO + 2SO2 (6.9) 2PbS + 3O2 → 2PbO + 2SO2 (6.10) 2Cu2S + 3O2 → 2Cu2O + 2SO2 (6.11) The sulphide ores of copper are heated in reverberatory furnace. If the ore contains iron, it is mixed with silica before heating. Iron oxide ‘slags of ’* as iron silicate and copper is produced in the form of copper matte which contains Cu2S and FeS. FeO + SiO2 → FeSiO3 (6.12) (slag) The SO2 produced is utilised for manufacturing H2SO4 . (b) Reduction of oxide to the metal Reduction of the metal oxide usually involves heating it with some other substance acting as a reducing agent (C or CO or even another metal). The reducing agent (e.g., carbon) combines with the oxygen of the metal oxide. MxOy + yC → xM + y CO (6.13) Some metal oxides get reduced easily while others are very difficult to be reduced (reduction means electron gain or electronation). In any case, heating is required. To understand the variation in the temperature requirement for thermal reductions (pyrometallurgy) and to predict which element will suit as the reducing agent for a given metal oxide (MxOy), Gibbs energy interpretations are made. Some basic concepts of thermodynamics help us in understanding the theory of metallurgical transformations. Gibbs energy is the most significant term here.The change in Gibbs energy, ΔG for any process at any specified temperature, is described by the equation: ΔG = ΔH – TΔS (6.14) where, ΔH is the enthalpy change and ΔS is the entropy change for the process. For any reaction, this change could also be explained through the equation: ΔGV = – RTlnK (6.15) where, K is the equilibrium constant of the ‘reactant – product’ system at the temperature,T. A negative ΔG implies a +ve K in equation 6.15. And this can happen only when reaction proceeds towards products. From these facts we can make the following conclusions: * During metallurgy, ‘flux’ is added which combines with ‘gangue’ to form ‘slag’. Slag separates more easily from the ore than the gangue. This way, removal of gangue becomes easier. 1. When the value of ΔG is negative in equation 6.14, only then the reaction will proceed. If ΔS is positive, on increasing the temperature (T), the value of TΔS would increase (ΔH < TΔS) and then ΔG will become –ve. 2. If reactants and products of two reactions are put together in a system and the net ΔG of the two possible reactions is –ve, the overall reaction will occur. So the process of interpretation involves coupling of the two reactions, getting the sum of their ΔG and looking for its magnitude and sign. Such coupling is easily understood through Gibbs energy (ΔGV) vs T plots for formation of the oxides (Fig. 6.4). The reducing agent forms its oxide when the metal oxide is reduced. The role of reducing agent is to provide ΔGV negative and large enough to make the sum of ΔGV of the two reactions (oxidation of the reducing agent and reduction of the metal oxide) negative. As we know, during reduction, the oxide of a metal decomposes: MxO(s) → xM (solid or liq) +21O2 (g) (6.16) The reducing agent takes away the oxygen. Equation 6.16 can be visualised as reverse of the oxidation of the metal. And then, the Δf GV value is written in the usual way: xM(s or l) + →O(g) M22x1O(s) [ΔGV(M,MO)] (6.17)xIf reduction is being carried out through equation 6.16, the oxidation of the reducing agent (e.g., C or CO) will be there: C(s) +21O2(g) → CO(g) [ΔG(C, CO)] (6.18) 21O2(g) → CO2(g) [ΔG(CO, CO2)]CO(g) + (6.19) If carbon is taken, there may also be complete oxidation of the element to CO2: 1 2C(s) +1 2O2(g) →1 2CO2(g) [1 2ΔG(C, CO2)] (6.20) On subtracting equation 6.17 [it means adding its negative or the reverse form as in equation 6.16] from one of the three equations, we get: MxO(s) + C(s) → xM(s or l) + CO(g) (6.21) MxO(s) + CO(g) → xM(s or l) + CO2(g) (6.22) MxO(s) +1 2C(s) → xM(s or l) +1 2CO2(g) (6.23) These reactions describe the actual reduction of the metal oxide, MxO that we want to accomplish. The ΔrG0 values for these reactions in general, can be obtained by similar subtraction of the corresponding Δf G0 values. As we have seen, heating (i.e., increasing T) favours a negative value of ΔrG0. Therefore, the temperature is chosen such that the sum of ΔrG0 in the two combined redox process is negative. In ΔrG0 vs T plots, this is indicated by the point of intersection of the two curves (curve for MxO and that for the oxidation of the reducing substance). After that point, the ΔrG0 value becomes more negative for the combined process including the reduction of MxO. The difference in the two ΔrG0 values after that point determines whether reductions of the oxide of the upper line is feasible by the element represented by the lower line. If the difference is large, the reduction is easier. 6.4.1 Applications (a) Extraction of iron from its oxides Oxide ores of iron, after concentration through calcination/roasting (to remove water, to decompose carbonates and to oxidise sulphides) are mixed with limestone and coke and fed into a Blast furnace from its top. Here, the oxide is reduced to the metal. Thermodynamics helps us to understand how coke reduces the oxide and why this furnace is chosen. One of the main reduction steps in this process is: FeO(s) + C(s) → Fe(s/l) + CO (g) (6.24) It can be seen as a couple of two simpler reactions. In one, the reduction of FeO is taking place and in the other, C is being oxidised to CO: FeO(s) → Fe(s) +21O2(g) [ΔG(FeO, Fe)] (6.25) C(s) +21O2 (g) → CO (g) [ΔG (C, CO)] (6.26) When both the reactions take place to yield the equation (6.24), the net Gibbs energy change becomes: ΔG (C, CO) + ΔG (FeO, Fe) = ΔrG (6.27) Naturally, the resultant reaction will take place when the right hand side in equation 6.27 is negative. In ΔG0 vs T plot representing reaction 6.25, the plot goes upward and that representing the change C→CO (C,CO) goes downward. At temperatures above 1073K (approx.), the C,CO line comes below the Fe,FeO line [ΔG (C, CO) < ΔG(Fe, FeO)]. So in this range, coke will be reducing the FeO and will itself be oxidised to CO. In a similar way the reduction of Fe3O4 and Fe2O3 at relatively lower temperatures by CO can be explained on the basis of lower lying points of intersection of their curves with the CO, CO2 curve in Fig. 6.4. In the Blast furnace, reduction of iron oxides takes place in different temperature ranges. Hot air is blown from the bottom of the furnace and coke is burnt to give temperature upto about 2200K in the lower portion itself. The burning of coke therefore supplies most of the heat required in the process. The CO and heat moves to upper part of the furnace. In upper part, the temperature is lower and the iron oxides (Fe2O3 and Fe3O4) coming from the top are reduced in steps to FeO. Thus, the reduction reactions taking place in the lower temperature range and in the higher temperature range, depend on the points of corresponding intersections in the ΔrG0 vs T plots. These reactions can be summarised as follows: At 500 – 800 K (lower temperature range in the blast furnace)– 3 Fe2O3 + CO → 2 Fe3O4 + CO2 (6.28) Fe3O4 + 4 CO → 3Fe + 4 CO2 (6.29) Fe2O3 + CO → 2FeO + CO2 (6.30) At 900 – 1500 K (higher temperature range in the blast (6.31) (6.32) Limestone is also decomposed to CaO which removes silicate impurity of the ore as slag. The slag is in molten state and separates out from iron. The iron obtained from Blast furnace contains about 4% carbon and many impurities in smaller amount (e.g., S, P, Si, Mn). This is known as pig iron and cast into variety of shapes. Cast iron is different from pig iron and is made by melting pig iron with scrap iron and coke using hot air blast. It has slightly lower carbon content (about 3%) and is extremely hard and brittle. Further Reductions Wrought iron or malleable iron is the purest form of commercial iron and is prepared from cast iron by oxidising impurities in a reverberatory furnace lined with haematite. This haematite oxidises carbon to carbon monoxide: (b) Extraction of copper from cuprous oxide [copper(I) oxide] In the graph of ΔrG0 vs T for formation of oxides (Fig. 6.4), the Cu2O line is almost at the top. So it is quite easy to reduce oxide ores of copper directly to the metal by heating with coke (both the lines of C, CO and C, CO2 are at much lower positions in the graph particularly after 500 – 600K). However most of the ores are sulphide and some may also contain iron. The sulphide ores are roasted/smelted to give oxides: 2Cu2S + 3O2 → 2Cu2O + 2SO2 (6.34) The oxide can then be easily reduced to metallic copper using coke: Cu2O + C → 2 Cu + CO (6.35) In actual process, the ore is heated in a reverberatory furnace after mixing with silica. In the furnace, iron oxide ‘slags of’ as iron silicate and copper is produced in the form of copper matte. This contains Cu2S and FeS. FeO + SiO2 → FeSiO3 (6.36) (Slag) Copper matte is then charged into silica lined convertor. Some silica is also added and hot air blast is blown to convert the remaining 6.5 Electrochemical Principles of Metallurgy FeS, FeO and Cu2S/Cu2O to the metallic copper. Following reactions take place: 2FeS + 3O2 → 2FeO + 2SO2 (6.37) FeO + SiO2 → FeSiO3 (6.38) 2Cu2S + 3O2 → 2Cu2O + 2SO2 (6.39) 2Cu2O + Cu2S → 6Cu + SO2 (6.40) The solidified copper obtained has blistered appearance due to the evolution of SO2 and so it is called blister copper. (c) Extraction of zinc from zinc oxide The reduction of zinc oxide is done using coke. The temperature in this case is higher than that in case of copper. For the purpose of heating, the oxide is made into brickettes with coke and clay. coke,1673KZnO + C Zn + CO (6.41) The metal is distilled off and collected by rapid chilling. We have seen how principles of thermodyamics are applied to pyrometallurgy. Similar principles are effective in the reductions of metal ions in solution or molten state. Here they are reduced by electrolysis or by adding some reducing element. In the reduction of a molten metal salt, electrolysis is done. Such methods are based on electrochemical principles which could be understood through the equation, ΔG0 = – nE0F (6.42) here n is the number of electrons and E0 is the electrode potential of the redox couple formed in the system. More reactive metals have large negative values of the electrode potential. So their reduction is difficult. If the difference of two E0 values corresponds to a positive E0 and consequently negative ΔG0 in equation 6.42, then the less reactive metal will come out of the solution and the more reactive metal will go to the solution, e.g., Cu2+ (aq) + Fe(s) → Cu(s) + Fe2+ (aq) (6.43) In simple electrolysis, the Mn+ ions are discharged at negative electrodes (cathodes) and deposited there. Precautions are taken considering the reactivity of the metal produced and suitable materials are used as electrodes. Sometimes a flux is added for making the molten mass more conducting. Aluminium In the metallurgy of aluminium, purified Al2O3 is mixed with Na3AlF6 or CaF2 which lowers the melting point of the mix and brings conductivity. The fused matrix is electrolysed. Steel vessel with lining of carbon acts as cathode and graphite anode is used. The overall reaction may be written as: 2Al2O3 + 3C → 4Al + 3CO2 (6.44) This process of electrolysis is widely known as Hall-Heroult process. Thus electrolysis of the molten mass is carried out in an electrolytic cell using carbon electrodes. The oxygen liberated at anode reacts with the carbon of anode producing CO and CO2. This way for each kg of Fig. 6.6: Electrolytic cell for the aluminium produced, about 0.5 kg of carbon extraction of aluminium anode is burnt away. The electrolytic reactions are: Cathode: Al3+ (melt) + 3e– → Al(l) (6.45) Anode: C(s) + O2– (melt) → CO(g) + 2e– (6.46) C(s) + 2O2– (melt) → CO2 (g) + 4e– (6.47) Copper from Low Grade Ores and Scraps Copper is extracted by hydrometallurgy from low grade ores. It is leached out using acid or bacteria. The solution containing Cu2+ is treated with scrap iron or H2 (equations 6.42; 6.48).Cu2+(aq) + H2(g) → Cu(s) + 2H+ (aq) (6.48) 6.6 Oxidation Reduction oxidation is the extraction of chlorine from brine (chlorine is abundant in sea water as common salt) . 2Cl–(aq) + 2H2O(l) → 2OH–(aq) + H2(g) + Cl2(g) (6.49) The ΔG0 for this reaction is + 422 kJ. When it is converted to E0 (using ΔG0 = – nE0F), we get E0 = – 2.2 V. Naturally, it will require an external e.m.f. that is greater than 2.2 V. But the electrolysis requires an excess potential to overcome some other hindering reactions. Thus, Cl2 is obtained by electrolysis giving out H2 and aqueous NaOH as byproducts. Electrolysis of molten NaCl is also carried out. But in that case, Na metal is produced and not NaOH. As studied earlier, extraction of gold and silver involves leaching the metal with CN–. This is also an oxidation reaction (Ag → Ag+ or Au → Au+). The metal is later recovered by displacement method. 4Au(s) + 8CN–(aq) + 2H2O(aq) + O2(g) → 4[Au(CN)2]–(aq) + 4OH–(aq) (6.50) 2[Au(CN)2]–(aq) + Zn(s) → 2Au(s) + [Zn(CN)4]2– (aq) (6.51) In this reaction zinc acts as a reducing agent. 6.7 Refining A metal extracted by any method is usually contaminated with some impurity. For obtaining metals of high purity, several techniques are used depending upon the differences in properties of the metal and the impurity. Some of them are listed below. (a) Distillation (b) Liquation (c) Electrolysis (d) Zone refining (e) Vapour phase refining (f) Chromatographic methods These are described in detail here. (a) Distillation This is very useful for low boiling metals like zinc and mercury. The impure metal is evaporated to obtain the pure metal as distillate. (b) Liquation In this method a low melting metal like tin can be made to flow on a sloping surface. In this way it is separated from higher melting impurities. (c) Electrolytic refining In this method, the impure metal is made to act as anode. A strip of the same metal in pure form is used as cathode. They are put in a suitable electrolytic bath containing soluble salt of the same metal. The more basic metal remains in the solution and the less basic ones go to the anode mud. This process is also explained using the concept of electrode potential, over potential, and Gibbs energy which you have seen in previous sections. The reactions are: M → Mn+Anode: + ne– Mn+– Cathode: + ne → M (6.52) Copper is refined using an electrolytic method. Anodes are of impure copper and pure copper strips are taken as cathode. The electrolyte is acidified solution of copper sulphate and the net result of electrolysis is the transfer of copper in pure form from the anode to the cathode: Anode: Cu → Cu2+ + 2 e– Cathode: Cu2+ + 2e– → Cu (6.53) Impurities from the blister copper deposit as anode mud which contains antimony, selenium, tellurium, silver, gold and platinum; recovery of these elements may meet the cost of refining. Zinc may also be refined this way. (d) Zone refining This method is based on the principle that the impurities are more soluble in the melt than in the solid state of the metal. A circular mobile heater is fixed at one end of a rod of the impure metal (Fig. 6.7). The molten zone moves along with the heater which is moved forward. As the heater moves forward, the pure metal crystallises out of the melt and the impurities pass on into the adjacent molten zone. The process is repeated several times and the heater is moved in the same direction. At one end, impurities get concentrated. This end is cut off. This method is very useful for producing semiconductor and other metals of very high purity, e.g., germanium, silicon, boron, (e) Vapour phase refining In this method, the metal is converted into its volatile compound and collected elsewhere. It is then decomposed to give pure metal. So, the two requirements are: (i) the metal should form a volatile compound with an available reagent, (ii) the volatile compound should be easily decomposable, so that the recovery is easy. Following examples will illustrate this technique. Mond Process for Refining Nickel: In this process, nickel is heated in a stream of carbon monoxide forming a volatile complex, nickel tetracarbonyl: 330 – 350 KNi + 4CO Ni(CO)4 (6.54) The carbonyl is subjected to higher temperature so that it is decomposed giving the pure metal: 450 –470KNi(CO)4 Ni + 4CO (6.55) van Arkel Method for Refining Zirconium or Titanium: This method is very useful for removing all the oxygen and nitrogen present in the form of impurity in certain metals like Zr and Ti. The crude metal is heated in an evacuated vessel with iodine. The metal iodide being more covalent, volatilises: Zr + 2I2 → ZrI4 (6.56) The metal iodide is decomposed on a tungsten filament, electrically heated to about 1800K. The pure metal is thus deposited on the filament. ZrI4 → Zr + 2I2 (6.57) (f) Chromatographic methods This method is based on the principle that different components of a mixture are differently adsorbed on an adsorbent. The mixture is put in a liquid or gaseous medium which is moved through the adsorbent. Different components are adsorbed at different levels on the column. Later the adsorbed components are removed (eluted) by using suitable solvents (eluant). Depending upon the physical state of the moving medium and the adsorbent material and also on the process of passage of the moving medium, the chromatographic method* is given the name. In one such method the column of Al2O3 is prepared in a glass tube and the moving medium containing a solution of the components is in liquid form. This is an example of column chromatography. This is very useful for purification of the elements which are available in minute quantities and the impurities are not very different in chemical properties from the element to be purified. There are several chromatographic techniques such as paper chromatography, column chromatography, gas chromatography, etc. Procedures followed in column chromatography have been depicted in Fig. 6.8. * Looking it the other way, chromatography in general, involves a mobile phase and a stationary phase. The sample or sample extract is dissolved in a mobile phase. The mobile phase may be a gas, a liquid or a supercritical fluid. The stationary phase is immobile and immiscible (like the Al2O3 column in the example of column chromatography above). The mobile phase is then forced through the stationary phase. The mobile phase and the stationary phase are chosen such that components of the sample have different solubilities in the two phases. A component which is quite soluble in the stationary phase takes longer time to travel through it than a component which is not very soluble in the stationary phase but very soluble in the mobile phase. Thus sample components are separated from each other as they travel through the stationary phase. Depending upon the two phases and the way sample is inserted/injected, the chromatographic technique is named. These methods have been described in detail in Unit 12 of Class XI text book (12.8.5). 6.8 Uses of Aluminium, Copper, Zinc and Iron Aluminium foils are used as wrappers for chocolates. The fine dust of the metal is used in paints and lacquers. Aluminium, being highly reactive, is also used in the extraction of chromium and manganese from their oxides. Wires of aluminium are used as electricity conductors. Alloys containing aluminium, being light, are very useful. Copper is used for making wires used in electrical industry and for water and steam pipes. It is also used in several alloys that are rather tougher than the metal itself, e.g., brass (with zinc), bronze (with tin) and coinage alloy (with nickel). Zinc is used for galvanising iron. It is also used in large quantities in batteries, as a constituent of many alloys, e.g., brass, (Cu 60%, Zn 40%) and german silver (Cu 25-30%, Zn 25-30%, Ni 40–50%). Zinc dust is used as a reducing agent in the manufacture of dye-stuffs, paints, etc. Cast iron, which is the most important form of iron, is used for casting stoves, railway sleepers, gutter pipes , toys, etc. It is used in the manufacture of wrought iron and steel. Wrought iron is used in making anchors, wires, bolts, chains and agricultural implements. Steel finds a number of uses. Alloy steel is obtained when other metals are added to it. Nickel steel is used for making cables, automobiles and aeroplane parts, pendulum, measuring tapes, chrome steel for cutting tools and crushing machines, and stainless steel for cycles, automobiles, utensils, pens, etc. in refining the metal. Metals, in general, are very widely used and have contributed significantly in the development of a variety of industries. Aluminium 1. Bauxite, Al2O3. x H2O 2. Cryolite, Na3AlF6 Electrolysis of Al2O3 dissolved in molten Na3AlF6 For the extraction, a good source of electricity is required. Iron 1. Haematite, Fe2O3 2. Magnetite, Fe3O4 Reduction of the oxide with CO and coke in Blast furnace Temperature approaching 2170 K is required. Copper 1. Copper pyrites, CuFeS2 2. Copper glance, Cu2S 3. Malachite, CuCO3.Cu(OH)2 4. Cuprite, Cu2O Roasting of sulphide partially and reduction It is self reduction in a specially designed converter. The reduction takes place easily. Sulphuric acid leaching is also used in hydrometallurgy from low grade ores. Zinc 1. Zinc blende or Sphalerite, ZnS 2. Calamine, ZnCO3 3. Zincite, ZnO Roasting followed by reduction with coke The metal may be purified by fractional distillation. Exercises 6.1 Copper can be extracted by hydrometallurgy but not zinc. Explain. 6.2 What is the role of depressant in froth floatation process? 6.3 Why is the extraction of copper from pyrites more difficult than that from its oxide ore through reduction? 6.4 Explain: (i) Zone refining (ii) Column chromatography. 6.5 Out of C and CO, which is a better reducing agent at 673 K ? 6.6 Name the common elements present in the anode mud in electrolytic refining of copper. Why are they so present ? 6.7 Write down the reactions taking place in different zones in the blast furnace during the extraction of iron. 6.8 Write chemical reactions taking place in the extraction of zinc from zinc blende. 6.9 State the role of silica in the metallurgy of copper. 6.10 What is meant by the term “chromatography”? 6.11 What criterion is followed for the selection of the stationary phase in chromatography? 6.12 Describe a method for refining nickel. 6.13 How can you separate alumina from silica in a bauxite ore associated with silica? Give equations, if any. 6.14 Giving examples, differentiate between ‘roasting’ and ‘calcination’. 6.15 How is ‘cast iron’ different from ‘pig iron”? 6.16 Differentiate between “minerals” and “ores”. 6.17 Why copper matte is put in silica lined converter? 6.18 What is the role of cryolite in the metallurgy of aluminium? 6.19 How is leaching carried out in case of low grade copper ores? 6.20 Why is zinc not extracted from zinc oxide through reduction using CO? 6.21 The value of ΔG0 for formation of CrO is – 540 kJmol−1and that of AlO isf2 3 2 3– 827 kJmol−1. Is the reduction of Cr2 O3 possible with Al ? 6.22 Out of C and CO, which is a better reducing agent for ZnO ? 6.23 The choice of a reducing agent in a particular case depends on thermodynamic factor. How far do you agree with this statement? Support your opinion with two examples. 6.24 Name the processes from which chlorine is obtained as a by-product. What will happen if an aqueous solution of NaCl is subjected to electrolysis? 6.25 What is the role of graphite rod in the electrometallurgy of aluminium? 6.26 Outline the principles of refining of metals by the following methods: (i) Zone refining (ii) Electrolytic refining (iii) Vapour phase refining 6.27 Predict conditions under which Al might be expected to reduce MgO. (Hint: See Intext question 6.4) Answers to Some Intext Questions 6.1 Ores in which one of the components (either the impurity or the actual ore) is magnetic can be concentrated, e.g., ores containing iron (haematite, magnetite, siderite and iron pyrites). 6.2 Leaching is significant as it helps in removing the impurities like SiO2, Fe2O3, etc. from the bauxite ore. 6.3 Certain amount of activation energy is essential even for such reactions which are thermodynamically feasible, therefore heating is required. 6.4 Yes, below 1350°C Mg can reduce Al2O3 and above 1350°C, Al can reduce MgO. This can be inferred from ΔGV Vs T plots (Fig. 6.4).